Abstract
The kinetics of the oxidation of acetone in the 'low-temperature’ region (i. e. below 320°C) have been carefully investigated. In contrast to the high-temperature region, the products include no methane, but appreciable quantities of methyl hydroperoxide as well as water, carbon monoxide and dioxide. A reaction scheme is suggested which involves degenerate chain branching by the homogeneous decomposition of methyl hydroperoxide. The transition from the low-temperature mechanism to that prevailing at high temperatures is due to the changing importance of the alternative reactions of the methyl radical. At low temperatures, the formation of methyl hydroperoxide is favoured CH
3
+ O
2
+
M
= CH
3
O
2
+
M
, CH
3
O
2
+
R
H = CH
3
O
2
H +
R
, whereas at high temperatures the methyl peroxy radical is too unstable to abstract hydrogen and instead the reaction yields formaldehyde CH
3
+ O
2
= HCHO + OH.
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